Question:
How many of the following have five radial nodes ?
5s, 6s, 7s, 6p and 4p
How many of the following have five radial nodes ?
5s, 6s, 7s, 6p and 4p
5s, 6s, 7s, 6p and 4p
Updated On: Feb 4, 2026
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Correct Answer: 6
Solution and Explanation
Calculation of Radial Nodes:
The number of radial nodes for an electron in an orbital is given by:
Radial nodes = n - l - 1,
where:
- n: Principal quantum number
- l: Azimuthal quantum number
Calculations for the given orbitals:
- 5s: \(n - l - 1 = 5 - 0 - 1 = 4\) radial nodes
- 6s: \(n - l - 1 = 6 - 0 - 1 = 5\) radial nodes
- 7s: \(n - l - 1 = 7 - 0 - 1 = 6\) radial nodes
- 6p: \(n - l - 1 = 6 - 1 - 1 = 3\) radial nodes
- 4p: \(n - l - 1 = 4 - 1 - 1 = 1\) radial node
Conclusion:
Only the 6s orbital has five radial nodes. Therefore, the correct answer is 6s.
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P-Block Elements
- P block elements are those in which the last electron enters any of the three p-orbitals of their respective shells. Since a p-subshell has three degenerate p-orbitals each of which can accommodate two electrons, therefore in all there are six groups of p-block elements.
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